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InterviewSolution
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Consider the following equilibrium: `SO_(3) rarr SO_(2)+O_(2)` `8.0 g` of `SO_(3)` are put in a container at `600^(@)C`. The equilibrium pressure and density are `1.8` atm and `1.6 g L^(-1)`, respectively a. Find the value of `K_(p)`. b. Also find the moles of helium that is to be added at equilibrium to double the pressure at constant temperature. |
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Answer» Weight of `SO_(3)` taken `=8.0 g` molecular weight of `SO_(3)=80 g//"mol"` `:.` mole of `SO_(3)=8/80=0.1 "mol"` `{:(SO_(3),hArr,SO_(2),+,1//2O_(2)),(0.1-x,,x,,x//2):}` `PV=nRT` or `PM=dRT` Total moles `=0.1+x//2` `rArr M=(dRT)/(P)=(1.6xx0.0821xx873)/(1.8)=63.6` `n_(1)M_(1)=n_(2)M_(2), n_(1)/n_(2)=M_(2)/M_(1)` `rArr (0.1)/(0.1+x//2)=M_(av)/M_(SO_(3))=63.6/80rArr x=0.05` `:. K_(p)=(((x//2)/(0.1+x//2)P)^(1//2)((xP)/(0.1+x//2)))/(((0.1-x)/(0.1+x//2)P))=0.61` `(P=1.8 "atm")` b. `n_(i)=0.1 x//2` To double pressure by adding inert gas at constant `T` double moles at equilibrium `rArr n_(f)=2(0.1+x//2)` `rArr n_(He)` added `=0.1+x//2=0.1+(0.05//2)=0.125` |
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